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Mole percent of O2 = 10% = 0.1 moles
Mole percent of N2 = 10% = 0.1 moles
Mole percent of He = 80% = 0.8 moles
Molar Mass of O2 = (2 x 16) x 0.1 = 3.2
Molar Mass of N2 = (2 x 14) x 0.1 = 2.8
Molar Mass of He = 4 x 0.8 = 3.2
1. Molar Mass of the mixture = 3.2 + 2.8 + 3.2 = 9.2 grams
2. Since at constant volume density is proportional to mass, so the ratio of
mass will be the ratio of density.
Ratio = Molar Mass of the mixture / Molar Mass of O2 = 9.2 / 32 = 0.2875
Answer:
- <u>Decreasing the temperature of the system will shift the reaction rightward.</u>
Explanation:
The complete question is:
Given the equation representing a system at equilibrium:
- N₂(g) + 3H₂(g) ⇌ 2NH₃(g) + energy
what changes occur when the temperature of this system is decreased?
<h2>Solution</h2>
Modifying the temperature of a system in equilibrium changes the equilibrium constant and the equilibrium position (concentrations) of the system.
When the temperature is decreased, following LeChatelier's principle that the system will react in a way that seeks to counteract the disturbance, the reaction will shift toward the reaction that produces more heat energy to compensate the temperature decrease.
Thus, decreasing the temperature of the system will favor the forward reaction, more N₂(g) and H₂(g) will be consumed and more NH₃(g) and energy will be produced. Hence, the equilibrium will shift rightward.
Molar mass = 144.2 g/mol.
<h3>Calculate
Molar mass.</h3>
Formula to solve this: ΔT = Kf . m
ΔT → Freezing point of pure solvent - Freezing point of solution
0°C - (-1.94°C) = 1.86 °C/m . m
1.94°C / 1.86 m/°C = m → 1.04 m
1.04 are the moles of solute in 1kg of solvent → molality (mol/kg)
Let's convert the mass of our solvent in kg to determine the moles.
80 g . 1kg / 1000 g = 0.08 kg
Molality . kg of solvent → Solute moles
1.04 mol/kg . 0.080 kg = 0.0832 moles
These are the moles of 12 g of solute. To find the molar mass → g/mol
12 g / 0.0832 mol = 144.2 g/mol
To learn more about Molar mass from the given link:
brainly.com/question/14787860
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Answer is: <span>the gas undergoes a chemical reaction that has fewer gas particles in products than in reactants. pressure is directly proportional to number of particles, so the pressure decreased.
Ideal gas law: PV = nRT. If amount of substance decreased, pressure also decreased.</span>
